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Chapter 47: Problem 7

Indicate which of the following are potential acids, potential bases, or both (potential acid and potential base). a) \(\mathrm{Al}^{3+}\) b) \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{+}\) c) \(\mathrm{HPO}_{4}^{2-}\) d) \(\quad \mathrm{F}^{-}\) e) \(\mathrm{NH}_{4}^{+}\) f) \(\mathrm{H}_{2} \mathrm{O}\)

Short Answer

Expert verified
a) \(\mathrm{Al}^{3+}\): Acid, b) \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{+}\): Acid, c) \(\mathrm{HPO}_{4}^{2-}\): Both acid and base, d) \(\mathrm{F}^{-}\): Base, e) \(\mathrm{NH}_{4}^{+}\): Acid, f) \(\mathrm{H}_{2} \mathrm{O}\): Both acid and base.

Step by step solution

01

Identifying potential acid - Al3+

\(\mathrm{Al}^{3+}\) has no hydrogen to donate but can accept electrons to fill its octet, so it can only act as an Lewis acid (electron acceptor). However, considering the Bronsted-Lowry definition, Al3+ cannot accept any more protons(H+), thus it is not a base.
02

Identifying potential acid - CH3NH3+

The species \(\mathrm{CH}_{3} \mathrm{NH}_{3}{ }^{+}\) already has an extra proton (H+), suggesting it can donate this proton and thus acts as an acid. But since it has no lone pairs, it cannot accept any more protons, so it is not a base.
03

Identifying potential acid/base - HPO4^2-

The species \(\mathrm{HPO}_{4}^{2-}\) can donate a proton, so it can act as an acid. It also has the capacity to accept a proton due to its negative charge, meaning it can also act as a base. Thus, HPO4^2- is both a potential acid and base.
04

Identifying potential base - F^-

The species \(\mathrm{F}^{-}\) has no proton to donate, but due to its negative charge, it can accept a proton (H+). So, it can be classified as a base.
05

Identifying potential acid - NH4+

The species \(\mathrm{NH}_{4}^{+}\) can donate a proton, and thus can act as an acid. However, it does not have any lone pair or negative charge to accept more protons, therefore, it is not a base.
06

Identifying potential acid/base - H2O

\(\mathrm{H}_{2} \mathrm{O}\) can both accept and donate a proton due to its hydrogen and lone pairs of electrons which can accept protons. So, it can act as both an acid and a base, making it an example of an amphoteric species.

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Most popular questions from this chapter

Describe how to determine the value of \(K_{\mathrm{b}}\) for a base-given the value of \(K_{\mathrm{a}}\) for its conjugate acid.

The chloride ion is the conjugate base of hydrochloric acid. Explain why \(\mathrm{Cl}^{-}\) does not produce a basic solution when dissolved in water.

Explain why the conjugate bases of the strong acids do not produce basic solutions when dissolved in water.

Consider two acids, HA and HX, with HA being a stronger acid than HX. a) Which acid has a larger value of \(K_{\mathrm{a}}\) ? b) Which conjugate base, \(\mathrm{A}^{-}\) or \(\mathrm{X}^{-}\), has a larger value of \(K_{\mathrm{b}}\) ? c) Provide a qualitative description of the relationship between the relative strength of an acid and the relative strength of its conjugate base.

Provide an expression relating \(K_{\mathrm{w}}\) to \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) of a conjugate acid-base pair.
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